Science 10 Course Review – Unit 1 Chemistry
Science 10- Course Review
Unit 1-Chemistry
Name ______
Date ______
Date due ______
The Science 10 Chemistry Unit covers:
Ø Chapter 8-Elements and the Periodic Table
Ø Chapter 9-Chemical Formulas and Compounds
Ø Chapter 10-Chemical Reactions
You can also consult the “Chemistry Outline” which shows all of the activities (Worksheets and Labs) If you don’t have one or if you want to view or print any of the activities, go to the Science 10 Web page at http://sd67.bc.ca/teachers/dcolgur and click “Science 10”
1. When zinc metal is placed in a solution of hydrochloric acid, it fizzes producing hydrogen gas and zinc chloride.
a) The reactants are ______
b) The products are ______
c) A word equation is: ______
2. In the following table, name the 3 major particles in the atom, state where they are located (in the nucleus or on the outside), state their relative mass compared to a proton (assume mass of a proton = 1) and their charge.
Particle / Location / Mass (Proton = 1) / Charge
3. List the four main points in John Dalton’s atomic theory.
1. ______
2. ______
3. ______
4. ______
4. Isotopes of an element are two different forms which have the same number of ______
and ______, but with different numbers of ______.
5. The atomic ______ of an element is the average mass of the isotopes which occur in nature.
6. In a neutral atom, the number of electrons is always equal to the number of
______or the ______number.
7. According to the model of the atom proposed by Neils Bohr, electrons move around the atom
in ______or ______. When one orbit is
filled, the electrons start filling the ______orbit.
8. The first orbit holds ______electrons.
The second orbit holds ______electrons.
The third orbit holds ______electrons.
9. Give the total number of electrons and the number of electrons in each orbit for each of the following elements:
Element / Total # ofelectrons / Electrons
in Level 1 / Electrons
in Level 2 / Electrons
in Level 3 / Electrons
in Level 4
Aluminum (Al)
Nitrogen (N)
Calcium (Ca)
Lithium (Li)
Argon (Ar)
10. Draw the Bohr models for neutral atoms of each of the following elements.
a) oxygen
b) chlorine
c) phosphorus
d) magnesium
11. According to Bohr, when a sample of an element is energized by heat or electricity, the
electrons jump to ______orbits. When they jump back down
to lower orbits, they give off the energy in the form of ______.
The amount of energy released in each jump corresponds to a certain ______
of light. The pattern of different colours of light given off is called the ______
for that element and can be seen through a device called a spectroscope. Because every element has its own set of electrons and orbits, the spectrum given off by each element will
be ______from that of any other element. What can this be used
for? ______
______
12. What are some practical uses for pure oxygen? ______
______
What is the main danger of pure oxygen? ______
13. Phosphorus is stored in ______. Suggest why? ______
______.
14. Why is phosphorus considered a dangerous element? ______
Suggest a practical use for elemental phosphorus ______
15. In order to have the same number of electrons as the noble gas neon, sodium
would have to ______electron.
Sodium is stored in ______. Suggest why? ______
______.
16. Is potassium more or less reactive than sodium ______. Find rubidium on your periodic table. Do you think rubidium would be more or less reactive
than potassium? ______.
17. Name iodine Symbol ______Atomic number _____ # of electrons _____
In order to have the same number of electrons as the noble gas xenon, iodine
would have to ______electron. Is iodine a metal or non-metal?______
18. Classify each of the following elements as an alkali metal, alkaline earth, halogen, noble gas or transition metal:
Element / FamilyFe
BrK
Kr
Ba
F
Pt
Li
Ne
Ra
19. Mendeleev arranged the elements in order of ______
and also put them in groups based on similar ______.
20. What did Mendeleev do when he came to a space where no known element would fit?
______
21. Vertical columns of the Periodic Table are known as Groups or Chemical ______.
22. Elements are no longer listed in order of atomic mass, but in order of atomic ______.
23. What is similar about elements in the same family? ______
24. What is the main use of helium? ______
25. What are some uses of argon? ______
26. Where is neon used? ______
27. Where are krypton and xenon used? ______
28. Why is the element radon considered dangerous even though it is not chemically reactive?
29. What would alkali metal atoms need to do in order to end up with the same stable electron
arrangements as the noble gases? ______
30. What can be said about the chemical reactivity of the alkali metals? ______
______
31. When alkali metals are put into water, what happens? ______
______
32. The outer orbits of halogen atoms each have ______electrons. This is one
(more/less) ______than the nearest noble gas atom.
33. In order to achieve the stable arrangement of noble gas atoms, each halogen atom would
have to ______electron.
34. Are the halogens metals or non-metals? ______
35. What can be said about the chemical reactivity of the halogens? ______
36. Why, other than reactivity, are halogens considered dangerous to work with? ______
37. Fill in the following table:
Indicators in Known Acids and Bases
Indicator / Colour in Acid / Colour in BasePhenolphthalein
Bromthymol Blue
Red Litmus
Blue Litmus
38. Are the pH’s of Acid Solutions < 7, >7 or = 7? ______
Are the pH’s of Base Solutions < 7, >7 or = 7? ______
39. The more acidic a solution is, the (lower/higher) the pH? ______
40. The more basic a solution is, the (lower/higher) the pH? ______
41. A solution with a pH = 7 is said to be ______
42. An acid HCl is mixed with a base KOH. Predict the chemical formulas for the two
products of this reaction. ______and ______. This
type of reaction of an acid reacting with a base is called ______
43. List 4 properties (characteristics) all acids have in common:
______
______
______
______
44. List 4 properties (characteristics) all bases have in common:
______
______
______
______
45. What is the name of the acid found in sour milk? ______
46. What is the name of the acid found in pop? ______
47. What is the name of the acid found in lemons and grapefruit? ______
48. What is the name of the acid found in your stomach? ______
49. What is the name of the acid found in car batteries? ______
50. What is the name of the acid found in rhubarb? ______
51. What is the name of the acid found in apples? ______
52. What is the name of the acid found in vinegar? ______
53. What is the name of the base found in oven cleaner? ______
54. Acid spills can sometimes be neutralized by which common compound? ______
______
55. Base spills can sometimes be neutralized by which common compound? ______
56. What is the chemical formula for common table salt? ______
57. What is the chemical name for baking soda? ______
58. What is the chemical formula for baking soda? ______
59. Which family of elements has just enough electrons in their highest orbits to
completely fill them up? ______
60. If Lithium is combined with Fluorine, the Lithium atom will ______an
electron to the Fluorine atom.
61. When Fluorine has gained an electron, it now has ____ protons (remember, it doesn’t lose
any protons), and ____ electrons. Because protons are positive (+) and electrons are
negative (-), the charge left over is _____. The Fluorine is no longer a neutral atom, but
is a charged atom, which is called a Fluoride ______.
62. Because the lithium ion (Li+) and the fluoride ion (F-) have opposite charges, they
______each other. This attraction forms an ______ic
bond.
63. Generally, combining capacity means the number of ______an atom
needs to lose or gain in order to have the same number of electrons as a ______
______.
64. The combining capacity of chromium (III) is ______
The combining capacity of manganese (IV) is ______
The combining capacity of iron (II) is .…...... ______
The combining capacity of copper (I) is ….... ______
65. Use the Periodic Table and the method shown to you by the teacher to write the correct formulas for the following ionic compounds.
a) magnesium iodide ......
______
b) aluminum fluoride ......
______
c) calcium sulphide ......
______
d) rubidium oxide ......
______
e) sodium phosphide ......
______
f) iron (III) sulphate ......
______
g) manganese (IV) oxide ......
______
h) copper (II) phosphate ......
______
i) calcium nitrate ......
______
j) ammonium chloride ......
______
k) lithium oxalate ......
______
l) nickel (III) carbonate ......
______
m) copper (I) permanganate ......
______
n) ammonium sulphate ......
______
66. Compounds with only two elements are called ______compounds.
67. In a binary compound, the non-metal changes it’s name so it ends in the letters ______.
68. In a compound containing a polyatomic ion, the name of the polyatomic ion
(always/sometimes/never)______changes.
69. Write the correct names for the following ionic compounds Spelling counts!
a) Na3PO4 ...... ______
b) K2S ...... ______
c) Rb2SO3 ...... ______
d) (NH4)2CO3 ...... ______
e) Ba(OH)2 ...... ______
f) MgSO4 ...... ______
g) Cs2HPO4 ...... ______
h) NaHCO3 ...... ______
i) AgNO3 ...... ______
j) Na3As ...... ______
k) NH4NO3 ...... ______
l) Ag2Cr2O7 ...... ______
70. In an ionic compound, electrons are ______from one atom
to the other. The element that lost electron(s) becomes a (+/-) ______ion and the
element than gains electron(s) becomes a (+/-) ______ion. The two oppositely charged
ions now (attract/repel) ______each other.
71. In a covalent compound, one atom ______electrons with another atom.
72. Show the Bohr model for a molecule of F2.
73. Give the formulas for molecules of the seven diatomic elements. The first one is H2.
______
74. Draw the Bohr model for a molecule of ammonia (NH3).
75. Write the correct formulas for the following covalent compounds:
a) nitrogen trioxide ...... ______
b) silicon tetrafluoride ...... ______
c) nitrogen monoxide ………………………… ______
d) selenium hexafluoride ...... ______
e) phosphorus pentachloride ...... ______
f) sulphur dioxide ...... ______
g) dinitrogen tetroxide ...... ______
76. Write the correct names for the following covalent compounds:
a) PF5 ...... ______
b) SO3 ...... ______
c) ClF6 ...... ______
d) SeO2...... ______
e) N2O ...... ______
f) N2Cl4 ...... ______
77. What is meant by a physical change? ______
Give 3 examples of physical changes:
______
______
______
78. What is meant by a chemical change? ______
Give 3 examples of chemical changes:
______
______
______
79. Balance the following equations by putting the proper coefficients wherever they are
needed.
a) Sr + O2 à SrO
b) Al + H2O à Al(OH)3 + H2
c) Al + O2 à Al2O3
d) C5H12 + O2 à CO2 + H2O
e) Na + H2O à H2 + NaOH
f) NaClO3 à NaCl + O2
g) Ca(NO3)2 + (NH4)2SO4 à CaSO4 + NH4NO3
h) C2H5OH + O2 à CO2 + H20
i) Al(NO3)3 + K2CrO4 à Al2(CrO4)3 + KNO3
j) NH3 à N2 + H2
k) C6H6 + O2 à CO2 + H2O
l) S8 + O2 à SO2
m) HNO3 + Fe(OH)3 à H2O + Fe(NO3)3
n) Br2 + CaCl2 à CaBr2 + Cl2
o) Mg + AlCl3 à MgCl2 + Al
Course Review – Unit 1 Chemistry Page 6